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3 years ago

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Calculate the concentration of the following solution in mol/dm3 0.1 moles of NaCl in 200 cm3

1 answer:

taurus [48]3 years ago

8 0

1 $cm ^{3}$ = 0.001 $dm ^{3}$ . Therefore 200 $cm ^{3}$ = 0.2 $dm ^{3}$ . Molarity = $\frac{number of moles of NaCl}{volume of the solution} = \frac{0.1}{0.2} = 0.5 mol/dm^{3}$ . Hope this helps.

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The three beakers shown below contain solutions of [cof6]3–, [co(nh3)6]3+, and [co(cn)6]3–. based on the colors of the three sol

vitfil [10]

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3 years ago

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3 years ago

E)¿Cuántos átomos de oxigeno hay en la molécula de glucosa, al reaccionar 12moleculas de agua?

elena55 [62]

Answer:

12 átomos de oxígeno hay presentes

Explanation:

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<em>6 moles de agua producen 1 mol de glucosa</em>

<em />

Si reaccionan 12 moleculas de agua, se producirán:

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2 moléculas de glucosa se producen.

Como cada molécula de glucosa tiene 6 átomos de oxígeno:

2 moléculas C₆H₁₂O₆ * (6 átomos Oxígeno / 1 molécula C₆H₁₂O₆) =

<h3>12 átomos de oxígeno hay presentes</h3>

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3 years ago

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Ivenika [448]

Answer:

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6 0

3 years ago

The heat of fusion AH, of ethyl acetate (C4H802) is 10.5 kinol. Calculate the change in entropy as when 398. g of ethy, acetate

Hitman42 [59]

<u>Answer:</u> The entropy change of the ethyl acetate is 133. J/K

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of ethyl acetate = 398 g

Molar mass of ethyl acetate = 88.11 g/mol

Putting values in above equation, we get:

$\text{Moles of ethyl acetate}=\frac{398g}{88.11g/mol}=4.52mol$

To calculate the entropy change for different phase at same temperature, we use the equation:

$\Delta S=n\times \frac{\Delta H_{fusion}}{T}$

where,

$\Delta S$ = Entropy change = ?

n = moles of ethyl acetate = 4.52 moles

$\Delta H_{fusion}$ = enthalpy of fusion = 10.5 kJ/mol = 10500 J/mol (Conversion factor: 1 kJ = 1000 J)

T = temperature of the system = $84.0^oC=[84+273]K=357K$

Putting values in above equation, we get:

$\Delta S=\frac{4.52mol\times 10500J/mol}{357K}\\\\\Delta S=132.9J/K$

Hence, the entropy change of the ethyl acetate is 133. J/K

7 0

3 years ago